SDS Volume (2687)
Volume 62. Carbon Dioxide in Water and Aqueous Electrolyte Solutions, p None
Original Measurements
Kobe, K. A.; Kenton, F. H.; Ind. Eng. Chem.; Anal. Ed. 1938, 10, 76-77.
Variables:
Room Temp:
298.15
$\pu{K}$
Pressure:
101.325
$\pu{kPa}$
Prepared by:
Method/Apparatus/Procedure:
The apparatus is described in detail in an earlier paper [1]. The apparatus consists of a gas buret, a pressure compensator, and a 200 mL absorption bulb and mercury leveling bulb. The absorption bulb is attached to a shaking mechanism.
The solvent and the gas are placed in the absorption bulb. The bulb is shaken until equilibrium is reached. The remaining gas is returned to the buret. The difference in the final and initial volume is taken as the volume of gas absorbed.
Source and Purity of Materials:
- Source not given. Purity stated to be 99+%.
- (2,3) Sources not given. Analytical grade.
- Distilled.
Estimated Errors:
Mass concentration (m/v) (1): δα/cm3 = ±0.005 (authors)
References
1 Kobe, K. A.; Williams, J. S.; Ind. Eng. Chem. 1935, 7 (1), 37-8.
Components:
- Carbon dioxide, $\ce{ CO2 }$; [124-38-9] NIST WebBook
- Sulfuric acid, $\ce{ H2SO4 }$; [7664-93-9] NIST WebBook
- Sodium sulfate, $\ce{ Na2SO4 }$; [7757-82-6] NIST WebBook
- Water, $\ce{ H2O }$; [7732-18-5] NIST WebBook
Experimental Data
The solvent is a mixture of
800 g H2O
200 g Na2SO4 (anhydrous)
40 ml H2SO4 (concentrated, c = 18 mol dm-3)
Thus the molality of the solution is
m2/mol kg-1 = 0.90 (H2SO4)
m3/mol kg-1 = 1.76 (Na2SO4)
| $T$ ($\pu{K}$) | $T$ (°C) | $L$ | α ($\pu{cm3(g) cm-3(l) atm-1}$) | V (1) ($\pu{cm3}$) | V (2) ($\pu{cm3}$) |
|---|---|---|---|---|---|
| 298.15 | 25 | 0.270 | 0.247 | 49.54 | 13.40 |
(a) Solvent volume.
(b) Carbon dioxide volume absorbed.
(c) Bunsen coefficient [cm3 (STP) cm-3 atm-1].
(d) Ostwald coefficient [cm3 cm-3]
